If $$ gas is bubbled through water at $293K$ , how

N2 exerts a partial pressure of bar If N2 gas is bubbled through water at 293 K, then number of millimoles of N2 that will dissolve in 1 L of water is?

If $$ gas is bubbled through water at $293K$ , how The correct answer is p=KH×=×103 bar×mol of O2mol of =×no2 x 18no2 =×10−3m mol of O2=1

N2 exerts a partial pressure of bar If N2 gas is bubbled through water at 293 K, then number of millimoles of N2 that will dissolve in 1 L of water is?

if i won the lottery i wouldn''t tell anyone Step 12 Calculate the partial pressure of O2 using the ideal gas law formula, PV = nRT, where P is the pressure, V is the volume,

If ${N_2}$ gas is bubbled through water at $293K$ , how many millimoles of ${N_2}$ gas would dissolve in $1Litre$ water Assuming that ${N_2}$ exerts a

ifa cfl Therefore, the number of millimoles of O2 gas that dissolve in 1 litre of water at 303 K when O2 gas is bubbled through it is 43 mmolL, which rounds off to

The number of millimoles of O2 gas that dissolve in 1 liter of water at 303 K is approximately 43 millimoles, calculated using Henry's Law and